Predict the shapes of the following molecules, and then...

Predict the shapes of the following molecules, and then predict which would have resultant dipole moments: (a) $\mathrm{SO}_{2} ;$ (b) $\mathrm{NH}_{3} ;$ (c) $\mathrm{H}_{2} \mathrm{S} ;$ (d) $\mathrm{C}_{2} \mathrm{H}_{4} ;$ (e) $\mathrm{SF}_{6}$; (f) $\mathrm{CH}_{2} \mathrm{Cl}_{2}$.

Key Concepts

VSEPR Theory

Valence Shell Electron Pair Repulsion (VSEPR) theory is a model used to predict the shape of individual molecules based on the repulsion between electron pairs surrounding a central atom. This theory explains how the arrangement of electrons determines molecular geometry, which in turn influences properties such as bond angles and molecular symmetry.

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms in a molecule. The specific shape, such as trigonal planar, tetrahedral, bent, trigonal pyramidal, or octahedral, depends on the number of bonding and lone pairs around a central atom. Understanding these geometries is critical for predicting chemical reactivity and physical properties.

Bond Polarity

Bond polarity is the result of differences in electronegativity between bonded atoms, creating areas of partial positive and negative charge. The individual bond dipoles contribute to the overall polarity of the molecule, and their vector summation determines whether the molecule has a net dipole moment.

Molecular Polarity and Dipole Moment

Molecular polarity arises when the vector sum of all bond dipoles in a molecule does not cancel out, resulting in a polar molecule with a permanent dipole moment. In contrast, symmetrical molecules may have polar bonds but be overall nonpolar because the individual dipole moments cancel each other out.

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